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Ch. 4 - Acids and Bases/Electron Flow
Mullins - Organic Chemistry: A Learner Centered Approach 1st Edition
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Mullins 1st EditionCh. 4 - Acids and Bases/Electron Flow문제 38d
3장, 문제 38d

Calculate Keq for these acid–base reactions.
(d)

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1
Step 1: Identify the acid and base on both sides of the reaction. In this case, the alcohol (CH3CH2OH) acts as the acid, and hydroxide ion (OH⁻) acts as the base. On the product side, the ethoxide ion (CH3CH2O⁻) is the conjugate base, and water (H2O) is the conjugate acid.
Step 2: Determine the pKa values of the acid and conjugate acid. The pKa of ethanol (CH3CH2OH) is approximately 16, and the pKa of water (H2O) is approximately 15.7.
Step 3: Use the relationship between pKa values and equilibrium constant (Keq). The formula is: Keq = 10^(pKa(conjugate acid) - pKa(acid)).
Step 4: Substitute the pKa values into the formula. Here, pKa(conjugate acid) = 15.7 (for H2O) and pKa(acid) = 16 (for CH3CH2OH).
Step 5: Calculate the exponent (pKa difference) and express the equilibrium constant (Keq) in terms of 10 raised to the power of the difference. This will give the final Keq value for the reaction.

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주요 개념

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Equilibrium Constant (K_eq)

The equilibrium constant, K_eq, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is calculated using the formula K_eq = [products]/[reactants], where the concentrations are raised to the power of their coefficients in the balanced equation. A K_eq greater than 1 indicates that products are favored, while a value less than 1 suggests that reactants are favored.
추천 영상:
02:19
The relationship between equilibrium constant and pKa.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In these reactions, acids donate protons, while bases accept them. Understanding the strength of acids and bases, often represented by their dissociation constants (K_a for acids and K_b for bases), is crucial for predicting the direction of the reaction and calculating K_eq.
추천 영상:
02:49
The Lewis definition of acids and bases.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium. This principle is essential in predicting how changes in concentration, pressure, or temperature will affect the position of equilibrium in acid-base reactions, thereby influencing the calculation of K_eq.
추천 영상:
04:12
The Electron Configuration
관련 실천
교과서 질문

For each indicated proton, suggest an approximate pKa value from Table 4.5. Rationalize your choice.

(b)

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교과서 질문

For each indicated proton, suggest an approximate pKa value from Table 4.5. Rationalize your choice.

(d)

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교과서 질문

Using qualitative reasoning for the acid–base reactions shown,

(i) which is stronger, the base or the conjugate base?

(ii) Which side of the reaction is favored?

(iii) Would you expect a Keq greater than or less than 1?

(a)

1191
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교과서 질문

Using qualitative reasoning for the acid–base reactions shown,

(i) which is stronger, the base or the conjugate base?

(ii) Which side of the reaction is favored?

(iii) Would you expect a Keq greater than or less than 1?

(c)

1001
views
교과서 질문

For the bases shown, draw the conjugate acid and identify a pKa value from Table 4.5 that would help you accurately estimate its stability.

(b)

1131
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교과서 질문

Calculate Keq for these acid–base reactions.

(c)

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